Two 30.0 mL samples, one 0.100M HCl and the other 0.100 M HF, weretitrated with 0.200 M KOH. Answer each of the tollowing questions regardingthese two titrations.Part APart CWhat is the volume of added base at the equivalence point for HCl?Express your answer in milliliters.Predict whether the pH at the equivalence point for each titration will be acidic, basic, or neutral.neutral for HCI, and acidic for HFneutral for HF, and acidic for HCImLneutral for HCl, and basic for HFneutral for HF, and basic for HCiSubmitRequest Answerneutral for bothPart BSubmitRequest AnswerWhat is the volume of added base at the equivalence point for HF?Part DExpress your answer in milliliters.Predict which titration curve will have the lower initial pH.HF curve10mLHCl curveSubmitPrevious Answers Request AnswerSubmitRequest AnswerX Incorrect; Try Again; 3 attempts remainingPart E Complete previous part(s)

A.) , B) Given acids are monoprotic ( Have one acidic H ) and base is KOH , so volume needed at…

Two 30.0 mL samples, one 0.100 M HCl and the other 0.100 M HF, wore titrated with 0.200 M KOH. Answer each of the following questions regarding these two titrations. • Part A Part C What is the volume of added base at the equivalence point for HCl? Express your answer in milliliters. Predict whether the pI at the equivalence point for each titration will be acidic, basic, or neutral. neutral for HCI, and acidic for HF neutral for HF, and acidic for HCI neutral for IICI, and basic tor HIF Submit Request Answer neutral for HF, and basic for HCI neutral for both Part B Submit Request Answer What is the volume of added base at the equivalence point for HF? Part D Express your answer in millilitere. Predict which titration curve will have the lower initial pH. ? O HF curve 10 mL O HCl curve

Two 30.0 mL samples, one 0.100 M HCl and the other 0.100 M HF, wore titrated with 0.200 M KOH. Answer each of the following questions regarding these two titrations. • Part A Part C What is the volume of added base at the equivalence point for HCl? Express your answer in milliliters. Predict whether the pI at the equivalence point for each titration will be acidic, basic, or neutral. neutral for HCI, and acidic for HF neutral for HF, and acidic for HCI neutral for IICI, and basic tor HIF Submit Request Answer neutral for HF, and basic for HCI neutral for both Part B Submit Request Answer What is the volume of added base at the equivalence point for HF? Part D Express your answer in millilitere. Predict which titration curve will have the lower initial pH. ? O HF curve 10 mL O HCl curve

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 50.0 mL solution of 0.179 M KOH is titrated with 0.358 M HCI. Calculate the pH of the solution after the addition of each of the given amounts of HCl. 0.00 mL pH = 13.25 7.00 mL pH = 13.05 12.5 mL pH = 12.875 20.0 mL pH = 12.41 24.0 mL pH = 11.67 9.82 25.0 mL pH = Incorrect 11.67 26.0 mL pH = 29.0 mL pH = Incorrect Incorrect
In order to determine the chloride concentration in a solution, a Mohr titration is perform. This involves adding a small amount of chromate to the solution and then slowly adding silver nitrate. Silver chloride is pale yellow solid while Silver chromate is a dark red. The appearance of the red silver chromate is the endpoint of the titration. Answer the questions below about this process. (Ksp of AgCl= 1.7x10^-10 and Ksp of Ag2CrO4= 1.12x10^-12) A 100 mL sample of water from a potentially contaminated stream is collected. A 0.0010 g of sodium chromate is dissolved in the sample. 1) if the solution had been 0.015 M in NaCl, what percent of the chloride is still in solution? Given the answer to the question above, it should be clear that "all" of the chloride is removed before the silver chromate appears. This is why we can use it as an endpoint. 2) if it requires 21.4 mL of a 0.1 M solution of silver nitrate to reach the equivalence point with 100 mL of solution, what was the original…
A 200.0 mL sample of 0.216 M strong acid is titrated with 0.170 M strong base. Determine the pH of the solution after the addition of 270.0 mL of strong base. 2.24 11.76 1.89 13.06 11.35
In an acid-base titration, a base or acid is gradually added to the other until they have completely neutralized each other. Since acids and bases are usually colorless (as are the water and salt produced in the neutralization reaction), pH is measured to monitor the reaction. Suppose that the equivalence point is reached after approximately 393 mL of a NaOH solution has been added (enough to react with all the acetic acid present) but that replicates are equally likely to indicate from 373 to 417 mL (exclusive), measured to the nearest mL. Assume that two technicians each conduct titrations independently. What is the probability that the average volume at equivalence from the technicians is 416 mL or 417? Select one: O a. 0.79069767 b. 0.00000000 c. 0.00054083 d. 1.00000000 e. 0.00049383 f. 0.02941176 O g. 0.04651163 O O
Use an acid-base titration to calculate the molar mass of an acıd. A 0.6758-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized barium hydroxide. The equivalence point in the titration is reached after the addition of 30.31 mL of 9.152x10 ² M barium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid. g/mol
Write the equation for the equilibirum that determines the pH at the following points in the titration curve of a weak acid (HA) being titrated with a strong base (OH) before any base has been added halfway to the equivalence point at the equivalence point
Using the pH of the solution, a student determined that their hydroxide concentration was 0.1972 M. Which of the following standardized HCl dilutions would be most appropriate for their titration? 1.006×10−1M HCl 1.206×10−5M HCl 1.401×10−3M HCl 1.312×10−4M HCl 1.197×10−2M HCl
Use the following two titration curves to answer each of the following statements. Select the choice that completes the statement correctly. 14 pH 7 0 Graph A 25 volume of titrant added (mL) In graph A, the end point occurs at a In graph B, the equivalence point occurs at a + 141 pH 7 0 Graph B 25 volume of titrant added (mL)
In the titration of a solution of weak monoprotic acid with a 0.1375 M solution of NaOH, the pH half way to the equivalence point was 4.46 . In the titration of a second solution of the same acid, exactly twice as much of a 0.1375 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
A buffer solution contains 0.100 M fluoride ions and 0.126 M hydrogen fluoride. What is the concentration (M) of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCI to 25.0 mL of this solution? Select one: Oa. 0.130 Ob. 0.122 OC. 0.0953 Od. 0.0900
A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.027 M HCI, and the equivalence point is reached after 38.1 mL of titrant are dispensed. Based on this data, what is the concentration (M) of the hydroxide ion? Type answer: 0.041
True or false? The pH of the titration of a weak base with a strong acid at equivalence point is higher than 7.00 and the solution is basic.